WELCOME TO AP CHEMISTRY 2012-2013 

 

Dear AP Chemistry Student: 

 

I hope you are ready for a fun, yet challenging year. You all have a very good 
background in basic chemistry from your Honors Chemistry class, but AP Chemistry is a 
little different. Rather than just memorizing how to do particular types of problems, you 
must instead really understand the chemistry concepts and be able to apply it to all sorts 
of different problems. Students who finish AP Chemistry come out with a much better 
understanding of the world around them as well as a great sense of accomplishment. AP 
Chemistry is a difficult class, but with motivation and effort, you will definitely succeed. 

 

The following packet is our first unit in AP Chemistry- Stoichiometry. We will be 
independently working out of this as part of your summer assignment. The work for this 
assignment is due the first day of class and will be graded for accuracy. We will 
have a quiz during the first week of school on the polyatomic ions and a test the 
following week of school on all of Unit 1. I encourage you to form a study group and 
begin by working on the summer assignment together. The course is much easier if you 
have a support system. Also, purchasing a AP Chemistry review book during the 
summer is highly recommended. This will be a useful supplement to the textbook that 
you will receive during the school year. 

 

If you are having problems on the assignment, please feel free to contact me at 
mshurleychem@gmail.com. Remember, this assignment is review of Chemistry I so if 
you are feeling overwhelmed you may want to talk to me about the pacing and structure 
of the course to see if it is a good fit for you. 

 

Have a great summer! Cant wait to work with you next year! 

 

Ms. Hurley 

 

 

 

Summer Assignment: 

. Complete packet provided. We will do the rest once school starts. 
. Where there are blank spots, you should take notes on that particular topic. Use 
your notes from Chemistry I or look around online. 
. Answer ALL questions and RECORD ON ANSWER SHEET provided. 
. Summer assignment is graded for accuracy. 
. Check out our class website: http://mshurleychemistry.weebly.com 
. Contact me if you need help. 


 


Name: ________________________ Summer Assignment Answers 

 

Review Significant Figures- include units 

 

1. _______________________ 

6. _______________________ 

2. _______________________ 

7. _______________________ 

3. _______________________ 

8. _______________________ 

4. _______________________ 

9. _______________________ 

5. _______________________ 

10. _______________________ 



 

Review Writing Formulas 

 

1. _______________________ 

9. _______________________ 

2. _______________________ 

10. _______________________ 

3. _______________________ 

11. _______________________ 

4. _______________________ 

12. _______________________ 

5. _______________________ 

13. _______________________ 

6. _______________________ 

14. _______________________ 

7. _______________________ 

15. _______________________ 

8. _______________________ 

16. _______________________ 



 

Review Naming Formulas 

 

1. _______________________ 

6. _______________________ 

2. _______________________ 

7. _______________________ 

3. _______________________ 

8. _______________________ 

4. _______________________ 

9. _______________________ 

5. _______________________ 

10. _______________________ 



 

Review Balancing, Classifying, and Writing Equations 

Balance 

Classification 

1. N2 + H2 . NH3 

__________________________ 

2. KClO3 . KCl + O2 

__________________________ 

3. AlBr3 + K2SO4 . KBr + Al2(SO4)3 

__________________________ 

4. C8H18 + O2 . CO2 + H2O 

__________________________ 

5. C3H8 + O2 . CO2 + H2O 

__________________________ 

6. Na + H2O . NaOH + H2 

__________________________ 



 

7. ______________________________________________________________________ 

 

8. ______________________________________________________________________ 


9. ______________________________________________________________________ 

 

10. _____________________________________________________________________ 

 

11. _____________________________________________________________________ 

 

12. _____________________________________________________________________ 

 

13. _____________________________________________________________________ 

 

14. _____________________________________________________________________ 

 

Review Mole Conversions 

 

1. _______________________ 

6. _______________________ 

2. _______________________ 

7. _______________________ 

3. _______________________ 

8. _______________________ 

4. _______________________ 

9a. _______________________ 

5. _______________________ 

9b. _______________________ 



 

Review Extended Mole Map 

 

1. _______________________ 

7. _______________________ 

2. _______________________ 

8. _______________________ 

3. _______________________ 

9. _______________________ 

4. _______________________ 

10. _______________________ 

5. _______________________ 

11. _______________________ 

6. _______________________ 

12. _______________________ 



 

Percent Composition 

 

1. ____________ 

3. ____________ 

5. ____________ 

2. ____________ 

4. ____________ 

6. ____________ 



 

Empirical Formula 

1. _______________________ 

5. _______________________ 

2. _______________________ 

6. _______________________ 

3. _______________________ 

7. _______________________ 

4. _______________________ 

8. _______________________ 



 


SUMMER ASSIGNMENT 2012 

Ms. Hurley 

General Information for Finding Significant Figures 

 

 

 

 

 

 

 

 

 

Rules for Calculations Using Significant Figures 

 

. When multiplying and dividing: 


 

 

. When adding and subtracting 


 

 

Perform the following calculations using the rules for significant figures. On the first 
line, write the unrounded calculation and on the second line, write the rounded 
calculation. 

 

1. 1.35 m x 2.467 m = __________ = ___________ 
2. 1035 m2  42 m = __________ = ___________ 
3. 12.01 mL + 35.2 mL + 6 mL = __________ = ___________ 
4. 55.46 g  28.9 g = __________ = ___________ 
5. 0.021 cm x 3.2 cm x 100.1 cm = __________ = ___________ 
6. 0.15 cm + 1.15 cm + 2.051 cm = __________ = ___________ 
7. 150 L3  4 L = __________ = ___________ 
8. 505 kg  450.25 kg = __________ = ___________ 
9. 1.252 mm x 0.115 mm x 0.012 mm = __________ = ___________ 
10. 1.278 x 103 m2  1.4267 x 102 m = __________ = ___________ 


**If you arent sure on the AP exam, use 3 significant figures!**


Memorizing Polyatomic Ions 

 

Memorizing the polyatomic ions is VERY important. You are expected to know them all 
year. 

 

For each of the 25 polyatomic ions listed below, you will make an index card. To save 
cards, cut each card in half. On one side of the card, write the name of the ion, on the 
other side write the formula and charge. Whenever you get a free moment, look at one 
side of the card and guess the other side. Have your mom, brother, friend quiz you with 
them. Keep doing this for one week and you should have them memorized. 

 

 

 

 

. Yes, you need to know both forms of acetate. 
. Hydrogen Carbonate is also called Bicarbonate. 
. You need to be able to go from the name to the ion (with the correct charges) and 
from the ion to the name. 
. Sometimes grouping them by charge helps. 
. Create your own practice quiz where you actually have to write your answers. 
This is much different than just flipping over flash cards. 


 

There will be a quiz on this during the first week of school. 


Review Writing Formulas From Names 

Notes: 

 

 

 

 

1. ammonium phosphate 9. iron II oxide 

2. iron III oxide 10. carbon monoxide 

3. calcium chloride 11. potassium nitrate 

4. magnesium hydroxide 12. aluminum sulfate 

5. copper II sulfate 13. lead IV chromate 

6. diphosphorus pentoxide . 14. potassium permanganate 

7. sodium hydrogen carbonate . 15. zinc nitrate 

8. aluminum sulfite 16. sodium thiocyanate 

 

Review Naming Ionic Compounds 

***Zinc+2 and Silver+1 do not need Roman Numerals*** 

 

1. FeSO4 6. FeCl3 

2. CuC2H3O2 7. PbSO4 

3. Fe2O3 8. NaHSO4 

4. Ag2SO4 9. NiBr3 

5. ZnCO3 10. Al(OH)3 

 

Review Balancing, Classifying, and Writing Equations 

 

Balance and Classify the following Equations as Synthesis, Decomposition, Single 
Replacement, Double Replacement, and Combustion. 

1. N2 + H2 . NH3 

2. KClO3 . KCl + O2 

3. AlBr3 + K2SO4 . KBr + Al2(SO4)3 

4. C8H18 + O2 . CO2 + H2O 

5. C3H8 + O2 . CO2 + H2O 

6. Na + H2O . NaOH + H2 

 

 

Write the word equations below as chemical equations and balance. 

*Dont forget the diatomic elements* 

 

7. Zinc reacts with lead II nitrate to yield zinc nitrate and lead. 

 

8. Aluminium bromide reacts with chlorine to yield aluminum chloride and bromine. 


9. Sodium phosphate reacts with calcium chloride to yield calcium phosphate and 
sodium chloride. 

 

10. Potassium chlorate when heated yields potassium chloride and oxygen gas. 

 

11. Aluminum reacts with hydrochloric acid yields aluminum chloride and hydrogen gas. 

 

12. Calcium hydroxide reacts with phosphoric acid yields calcium phosphate and water. 

 

13. Copper reacts with sulfuric acid to yield copper II sulfate and water and sulfur 
dioxide. 

 

14. Hydrogen reacts with nitrogen monoxide to yield water and nitrogen. 

 

 

Review Mole Conversions 

 

Write the conversion factors on each line: 

 

 Mole 

 

 

 

 

 Mass (g) Particles (atoms, molecules) 

 Volume (L) 

 

 

Do the following conversions: 

1. 0.5 moles of C6H12O6 to grams 3. 100 g of KMnO4 to moles 

2. 35 g of CuSO4  5 H2O to moles 4. 3.2 moles of CuSO4  5 H2O to grams 

 

5. How many grams are there in 1.5 x 1025 molecules of CO2? 

 

 

6. A sample of NH3 gas occupies 75.0 liters at STP. How many grams is this? 

 

 

7. How many atoms are there in 1.3 x 1022 molecules of NO2? 

 

 

8. A 5.0 gram sample of O2 is in a container at STP. What volume is the container? 

 

 

9. a. How many molecules of O2 are in the container in Problem 8? b. How many atoms 
of oxygen? 


Review Extended Mole Map 

Mole: Mole Calculations 

 

Fill in the conversion factors on the lines. 

 

 g A g B 

 

 

 

 L A Mole A Mole B L B 

 

 

 

Particles A Particles B 

 

Example: Given the formula: N2 + 3 H2 
. 2 NH3, how many grams of NH3 will be 
produced if 67.2 L of N2 reacts with excess H2? 

 

Steps: L N2 . moles N2 . moles NH3 . g NH3 (Ignore excess) 

 

67.2 L N2 x 

 1 mole N2 x 

 2 mole NH3 x 

 17 g NH3 

 

 22.4 L N2 

 1 mole N2 

1 mole NH3 



 

 Practice: 

 

1. 2KClO3 . 2KCl + 3O2 

How many grams of potassium chloride are produced if 25 g of potassium chlorate decompose? 

 

 

 _______________ 

2. N2 + 3H2 . 2NH3 

How many grams of hydrogen are necessary to react completely with 50.0 g of nitrogen? 

 

 

 _______________ 

3. How many grams of ammonia are produced from 50.0 g of nitrogen? 

 

 

 _______________ 

4. 2AgNO3 + BaCl2 . 2AgCl + Ba(NO3)2 

How many grams of silver chloride are produced from 5.0 g of silver nitrate? 

 

 

 _______________ 

5. How much barium chloride is necessary to react with 5 g of silver nitrate? 

 

 

 _______________ 

 




6. N2 + 3H2 . 2NH3 

What volume of NH3 at STP is produced if 25.0 g of N2 is reacted with an excess of H2? 

 

 

 _______________ 

7. 2KClO3 . 2KCl + 3O2 

If 5.0 g of KClO3 is decomposed, what volume of O2 is produced at STP? 

 

 

 _______________ 

8. How many grams of KCl are produced from 5.0 g of KClO3? 

 

 

 _______________ 

9. Zn + 2HCl . ZnCl2 + H2 

What volume of hydrogen at STP is produced when 2.5 g of zinc react with an excess of 
hydrochloric acid? 

 

 

 _______________ 

10. H2SO4 + 2NaOH . H2O + Na2SO4 

How many molecules of water are produced if 2.0 g of sodium sulfate are produced? 

 

 

 _______________ 

11. 2AlCl3 . 2Al + 3Cl2 

If 10.0 g of aluminum chloride are decomposed, how many molecules of Cl2 are produced? 

 

 

 _______________ 

12. If 20.0 g of aluminum is produced, how many atoms of chlorine in AlCl3 reacted? Use the 
equation from problem 11. 

 

 

 _______________ 



 

Review- Percent Composition 

 

Formula: Mass of part  Mass of whole x 100 

 

1. Find the percent composition of oxygen in KMnO4. ___________________ 


 

2. Find the percent composition of hydrogen in (NH4)3PO4 ________________ 


 

3. Find the percent composition of nitrogen in Mg(NO3)2 _________________ 


 

4. How many grams of oxygen can be produced from the decomposition of 100 
grams of KClO3? 


 _________________ 


5. How much iron can be recovered from 25.0 g of Fe2O3? 


 

 _________________ 

6. How much silver can be produced from 125 g of AgS? 


 

 ________________ 

 

 

Review- Empirical and Molecular Formulas 

 

Empirical Formula- 

 

Molecular Formula- 

 

 Ex. C6H12O6 
. CH2O 

 Molecular Empirical 

Example 1: 

A compound with elements C, H, and O is found to have 9.1% hydrogen and 54.5% 
carbon. What is the empirical formula? 

 

Steps: 9.1 g H x (1 mole/ 1 g) = 9.1 mol / 2.275 = 4 H 

1. Assume 100 g 54.5 g C x (1 mol/ 12 g) = 4.5417 mol C / 2.275 = 2 C 

2. Convert to moles 36.4 g O x (1 mol/ 16 g) = 2.275 mol O /2.275 = 1 O 

3. Divide by smallest # moles C2H4O (put in alphabetical order) 

 

Example 2: 

A compound with an empirical formula of C2H4O has a molecular mass of 176 g/mol. 
What is the molecular formula? 

 

Step 1- complete chart for what you know: 

Molecular Formula 

Molecular Mass 

Empirical Formula 

Empirical Mass 

X Factor 

 

176 

C2H4O 

 

 



Step 2- Find the empirical mass. Divide the molecular mass by empirical mass to find 
X Factor 

Molecular Formula 

Molecular Mass 

Empirical Formula 

Empirical Mass 

X Factor 

 

176 

C2H4O 

44 

4 



Step 3- Distribute the x factor across the empirical: C8H16O4 

 

 

*Tips: 

- Carry decimal places out at least 4 digits 

- You can only round to a whole # if it is within 1 tenth of that #. (Ex. 1.03 . 1) 

- When you are not within 1 tenth you will need to multiply all of your answers so 
they are whole numbers. (Ex. 1.5 x 2 = 3; 1.2 x 5 = 6) 

 

Find the empirical formulas: 

1. 75% carbon, 25% hydrogen 

 

 




2. 52.7% potassium, 47.3% chlorine 

 

 

3. 32.4% sodium, 22.5% sulfur, 45.1% oxygen 

 

 

4. 25.3 % copper, 12.9% sulfur, 25.7% oxygen, 36.1% water 

 

 

5. 26.6% potassium, 35.3 % chromium, 38.1 % oxygen 

 

 

6. 56.4 % oxygen, 43.7 % phosphorus 

 

 

7. A compound is found to be 64.9 % carbon, 13.5% hydrogen, and 21.6% oxygen. Its 
molecular mass is 74 g/mol. What is its molecular formula? 

 

 

8. A compound is 54.5% carbon, 9.1% hydrogen, and 36.4% oxygen. Its molecular mass 
is 88 g/mol. What is its molecular formula? 

 

 



 

****End of Summer Assignment**** 

 

Miscellaneous: 

*You CANNOT use a calculator on the final exam! That means you need to be able to do 
math without it. 

 

Try these problems without using your calculator then check your answers. 

 

1. 34.99 + 20.098 
2. 890.111  768.942 
3. 43.9 x 10.12 
4. 45.6  13.4 
5. 35.9  0.15 
6. 2.33 x .54 


 

Start Memorizing these now!!! 

 

Flame Test Colors 

Li+ Deep red (crimson) 

Na+ Yellow 

K+ Violet 

Ca2+ Orange-red 

Sr2+ Red 

Ba2+ Green 

Cu2+ Blue-green 


Aqueous Ion Colors 

Cu1+ Green 

Cu2+ Blue 

Fe Yellow to red-orange (depending on anion and charge of Fe); 
in 
rare cases, can form complex ion with a deep blue color 

Fe2+ yellow-green (depending on the anion) 

Fe3+ orange-red (depending on the anion) 

MnO4- Purple (Mn w/ +7 oxidation state is purple) 

CrO42- Yellow 

Cr2O72- Orange 

Cu(NH3)42+ Dark Blue; produced when ammonia is added to Cu2+ 
solutions 

FeSCN2+ Red-brown, Wine-red to dark orange 

. Al, K, Li, Mg, Na, Ca, Ba, Sr, Zn are colorless aqueous ions and most of their 
solid salts are white. 
. Transition element ions with partially filled d orbitals tend to release colored 
light. 


 Assorted Compounds 

F2 Pale-yellow gas 

Cl2 Green-yellow gas 

Br2 Red-brown liquid 

I2 Dark-violet vapor & dark metallic looking solid 

S8 Yellow, odorous solid 

NO Colorless gas; associated with reactions between metals and 
dilute HNO3 

NO2 Brown gas; associated with reactions between metals and 
concentrated HNO3 

PbI2 Bright yellow precipitate 

Metallic sulfides Sulfides of transition metals tend to be black 

Fe2O3 Reddish brown (rust) 

Metallic oxides Oxides of colored transition metal ions tend to be colored 

 

Acid-Base Indicators 

Phenolphthalein Colorless (pH<7) to Pink (pH>8 ; when OH- is present) 

Red Litmus (paper) Turns purple in alkaline solution 

Blue Litmus (paper) Turns pink in acidic solution 

 

Courtesy Scott Halander 
Westview HS, SD, CA 

 

 

 

 

 

 


Solubility Rules- MEMORIZE NOW! 

 

Ion Formula 

Ion Name 

Mostly Soluble? 

Except 

Group 1 

Alkali Metals 

Yes- ALWAYS 

N/A 

NH4+ 

Ammonium 

Yes- ALWAYS 

N/A 

NO3- 

Nitrate 

Yes- ALWAYS 

N/A 

ClO3- 

Chlorate 

Yes- ALWAYS 

N/A 

ClO4- 

Perchlorate 

Yes- ALWAYS 

N/A 

C2H3O2- 

Acetate 

Yes- ALWAYS 

N/A 

Cl-, Br-, I- 

Chlorides, 
bromides, iodides 

Yes 

When combined with Ag+, 
Pb+2, Hg2+2 they are insoluble 

SO4-2 

Sulfates 

Yes 

When combined with Ag+, 
Pb+2, Hg2+2, Ca+2, Sr+2, Ba+2 
they are insoluble 

OH- 

Hydroxides 

No 

When combined with alkali 
metals, Ca+2, Sr+2, Ba+2 
they are 
soluble 

CO3-2 

Carbonates 

No 

When combined with alkali 
metals and ammonium they are 
soluble 

PO4-3 

Phosphates 

No 

When combined with alkali 
metals and ammonium they are 
soluble 

SO3-2 

Sulfites 

No 

When combined with alkali 
metals and ammonium they are 
soluble 

CrO4-2 

Chromates 

No 

When combined with alkali 
metals and ammonium they are 
soluble 

S-2 

Sulfides 

No 

When combined with alkali 
metals, alkali earth metals, and 
ammonium they are soluble 



 

 


